EP0629177A1 - Procede pour la production du dioxyde de chlore - Google Patents

Procede pour la production du dioxyde de chlore

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Publication number
EP0629177A1
EP0629177A1 EP93907256A EP93907256A EP0629177A1 EP 0629177 A1 EP0629177 A1 EP 0629177A1 EP 93907256 A EP93907256 A EP 93907256A EP 93907256 A EP93907256 A EP 93907256A EP 0629177 A1 EP0629177 A1 EP 0629177A1
Authority
EP
European Patent Office
Prior art keywords
acid
chlorite
chlorine dioxide
salt
amount
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Withdrawn
Application number
EP93907256A
Other languages
German (de)
English (en)
Other versions
EP0629177A4 (fr
Inventor
Habib Roozdar
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
ARCO RESEARCH Inc
Original Assignee
ARCO RESEARCH Inc
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by ARCO RESEARCH Inc filed Critical ARCO RESEARCH Inc
Publication of EP0629177A1 publication Critical patent/EP0629177A1/fr
Publication of EP0629177A4 publication Critical patent/EP0629177A4/fr
Withdrawn legal-status Critical Current

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B11/00—Oxides or oxyacids of halogens; Salts thereof
    • C01B11/02—Oxides of chlorine
    • C01B11/022—Chlorine dioxide (ClO2)
    • C01B11/023—Preparation from chlorites or chlorates
    • C01B11/024—Preparation from chlorites or chlorates from chlorites

Definitions

  • the present invention relates to a method for produc ⁇ ing chlorine dioxide (CIO2) disinfecting solution which preferably minimizes the amount of residual chlorite ion (C10 2 ”) so that the disinfecting solution can be used in the food, food processing, drinking water, pharmaceutical produc ⁇ tion and medical and dental related industries.
  • CIO2 chlorine dioxide
  • C10 2 residual chlorite ion
  • the present invention also relates to a method for generation of chlorine dioxide (CIO2) in low acidity disin ⁇ fecting compositions which suitable for applications where corrosion, a pH related property, is a concern and is required to be either prevented or minimized so that the disinfecting composition can be used in the treatment of metal-containint substrates such as dental and medical instruments and devices.
  • CIO2 chlorine dioxide
  • Chlorine dioxide an indirect food additive, has been found to be especially useful as a disinfectant, antiseptic and sanitizer. It is widely used to disinfect drinking water and various water supplies. In addition, chlorine dioxide finds use as a bleaching agent for flour, fats, textiles and as an antiseptic.
  • chlorine dioxide can not be transported commercially as a con ⁇ centrated gas for its use and instead has been generated at the site where it is used.
  • Chlorine dioxide has shown great utility as an antiseptic for treating metal substrates such as dental and medical instruments and devices.
  • meth ⁇ ods for generating chlorine dioxide suffer from the disad ⁇ vantage that large quantities of chlorite remain as a residue.
  • Chlorite residues on food handling equipment and medical and dental surfaces that are to come in contact with humans are to be avoided or substantially minimized according to FDA and EPA regulations.
  • chlorine dioxide exhibits certain cor ⁇ rosive properties which are believed to be pH related. Thus, it is beneficial to generate chlorine dioxide at a pH which would avoid or minimize corrosion during the disinfecting process.
  • the generated pool of chlorous acid is in equilibrium with the chlorite ion and not the strong acid, because the original acid is almost entirely ionized at the pH employed and hence has shifted the equi ⁇ librium toward formation of chlorous acid.
  • the hydrogen ion concentration from use of a relatively strong acid will produce optimal concentrations of chlorous acid.
  • the gen ⁇ erated chlorous acid has less of a tendency to ionize because the conjugate base of the original acid is not powerful enough to compete for the hydrogen ions.
  • the lower the pKa of the acid less acid is needed to generate chlorous acid.
  • Sulfuric acid for example, is corrosive, a powerful oxidizing agent and therefore, dangerous.
  • Nitric acid is similar to sulfuric acid and may produce nitrosamine residues, which are carcinogenic.
  • Hydrochloric acid is corrosive due to the chloride ion which alo tends to favor the production of chlorate anion, an unfavorable result (4) .
  • Figure 1 is a diagrammatic representation of a system for producing chlorine dioxide from a salt of a chlorite and an acid, preferably a biologically compatible acid and optionally, a disproportionation agent.
  • the reaction(s) to form chlorine dioxide occurs in the reaction chamber (C) .
  • the pipes, chambers and vats as set forth in Figure 1 are generally made of high density polyethylene and/or polypropylene.
  • Figure 2 is a diagrammatic representation of a two- part system comprising two containers, one for chlorite salt and the other for the acid.
  • the two parts could be considered as two separate containers, with or without dispensing pumps.
  • a measuring cup can be used for removing approximately equal volumes of the chlorite part and the acid part .
  • salt of a chlorite or "chlorite salt” is used throughout the specification to describe a salt of chlorite which is readily soluble in an aqueous system and which readily dissociates into chlorite anion and counterion (generally, metal) .
  • chlorite salts include sodium chlorite and potassium chlorite.
  • low pKa acid non-toxic low pKa acid
  • biologically compatible low pKa acid is used throughout the specification to describe acids which are relatively strong (have pKa's of about 2.1 or lower, preferably below about 1.94, the pKa of chlorous acid so as to shift the equilibrium to chlorous acid generation) and are easily or relatively safely handled, are generally compatible with biological systems (they are substantially non-toxic) and are non- caustic.
  • Low pKa acids donate a large fraction of hydrogen ions by favoring a reaction which consumes hydrogen ions and favors the generation of chlorine dioxide.
  • the acids utilized in the present invention are highly ionized and smaller quantities of the low pKa acid would be needed to protonate chlorite ions to form chlorous acid. Consequently, the acids have low residual levels.
  • the residues that are formed from these biologically compatible acids are generally the sodium and/or potassium salts of the acids, such residues being safe, non-corrosive and acceptable as either direct or indirect food additives.
  • biologically compatible or non-toxic acids for use in the present invention include sodium and potassium bisul ⁇ fate (NaHS(_> 4 and KHSO4) , phosphoric acid and maleic acid.
  • the bisulfates have pKa's of about 1.9-2.0, phosphoric acid has a pKa of about 2.15 and maleic acid has a pKa of about 1.94.
  • Other biologically compatible acids which may be used in the present invention include phosphoric acid. ethylenediaminetetraacetic acid (EDTA, as the free acid or the monosodium salt) among others.
  • hydrochloric, nitric and concentrated sulfuric acid or sulfuric acid in its free acid form are not considered biologically compatible acids for purposes of the present invention because of their caustic nature and their resultant difficulty in handling.
  • these acids may be used, preferably in diluted form.
  • chlorous acid disproportionation agent "disproportionation agent” or “aldehyde agent” is used throughout the specification to describe a number of dis ⁇ proportionation agents which enhance the rate of dis ⁇ proportionation of chlorous acid to produce significantly increase the amount of chlorine dioxide which is produced and minimizes residual chlorite ion.
  • the disproportion agents according to the present invention are chosen for their ability to substantially enhance the rate and efficiency (yield) at which chlorine dioxide is formed from chlorous acid (even at relatively high pH's and low concentrations of acid- a consideration in the embodiments which minimize corrosion) , for their ability to form their biologically compatible sub ⁇ stantially non-toxic organic acid side products and for their ability to minimize residual chlorite ion.
  • a disproportionation agent according to the present invention, one can produce effective quantities of CIO 2 , minimize the amount of acid used, raise the pH of the CIO2-generating solu ⁇ tion to a non-corrosive level, if desired,
  • Disproportionation agents for use in the present invention include, for example, substantially non-toxic aldehydes such as acetaldehyde , benzaldehyde, glutaraldehyde, cinnamic aldehyde, propionaldehyde, paraldehyde, 2-Furfural (bran oil) and 5-Hydroxymethyl-2-furfural (5HMF) , among others.
  • Preferred disproportionation agents for use in the present invention include those aldehydes that are substan ⁇ tially non-toxic themselves and which are converted during the disproprotionation process to substantially non-toxic side products.
  • Acetaldehyde, benzaldehyde, cinnamic aldehyde, glutaraldehyde and propionaldehyde are particularly preferred for use in the present invention.
  • corrosive properties is used throughout the specification to describe properties such as those producing corrosion on metal substrates such as medical and/or dental devices. These properties are derived from factors such as excess residual acidity (low pH) and/or excess residual chlorite ion.
  • enhanced chlorous acid disproportionation is used throughout the specification to describe the produc ⁇ tion of chlorine dioxide from chlorous acid in the presence of a disproproportionation agent such as an aldehyde, a combina ⁇ tion which has a faster rate and greater efficiency of chlorite ion use even when the pH is less acidic and which generally produces chlorine dioxide in greater amounts and at higher concentrations than without a disproportionation agent.
  • a disproportionation agent such as an aldehyde
  • the amount of chlorine dioxide which is generated in a reaction at a pH of about 3.9 during a 15 minut period is generally no greater than about 1-2 parts per million. This indicates that the rate of conversion of chlorous acid to chlorine dioxide in this case is very slow and the yields are low. In addition, residual acid remains, thus increasing the potential for producing corrosion.
  • the amount of chlorine dioxide generated may be as much as about 40 ppm or more.
  • hydrogen ions and residual chlorite ions are consumed by the disproportionation of chlorous acid, such that at the end of a 15 minute period, the pH rises to about 4.3.
  • This more effecient process for producing chlorine dioxide results in chlorite ion levels being substantially reduced relative to processes which generate chlorine dioxide in the absence of an aldehyde.
  • the residual chlorite ion levels are about 60% or less of the initial chlorite ion.
  • the terms “minimize residual chlorite ion”, “minimiz ⁇ ing residual chlorite ion” or “substantially reduce residual chlorite ion” are used throughout the specification to des ⁇ cribe reactions to produce chlorine dioxide which yield no more than about 85% by weight residual chlorite ion (based upon the initial weight of chlorite used) .
  • the amount of residual chlorite ion is less than about 70% by weight and most preferably the amount of residual chlorite ion is less than about 60% by weight.
  • substantially non-toxic is used throughout the specification to describe disproportionation agents and/or biologically compatible acids which are used to generate chlorine dioxide in the method(s) according to the present invention.
  • substantially non-toxic means that the materials are safely handled and are generally compatible with biologi ⁇ cal systems in amounts used to generate chlorine dioxide rela ⁇ tive to compositions which are considered “substantially toxic.”
  • substantially is used to describe the non- toxic acids and disproportionation agents for use in the pres ⁇ ent invention because of the fact that almost all substances, including water, may become toxic to a biological system in certain amounts.
  • substantially quantity is used to describe amounts of chlorine dioxide which are produced using the method according to the present invention and are believed to be useful.
  • a substantial quantity of chlorine dioxide for purposes of the present invention is at least about 1 part per million, because chlorine dioxide is a disinfectant at that concentration and higher concentrations.
  • chlorine dioxide is preferably produced in a con ⁇ centration of at least about 5 parts per million, most preferably at least about 20-40 parts per million.
  • low acidity composition and "high pH acid composition” are used throughout the disclosure to describe a chlorine dioxide-generating composition (producing at least about 1 ppm chlorine dioxide) and having a relatively low con ⁇ centration of acid to produce an initial pH of about 3.5 to about 4.5, and which comprises an amount of a water soluble salt of chlorite with an amount of a low pKa acid effective to produce a pH within the above range.
  • the composition may be dry or in solution.
  • chlorite part is used throughout the speci ⁇ fication to describe the form in which an amount of a water soluble salt of chlorite either in dry or liquid state is added to the acid part.
  • acid part is used throughout the specifica ⁇ tion to describe the form in which an amount of a water soluble low pKa acid either in dry or liquid state is added to the chlorite part.
  • low acidity condition is used throughout the specification to describe the condition at which at least 1 part per million (ppm) of chlorine dioxide is generated in a solution with a starting pH ranging from about 3.5 to about 4.5. This condition is provided by combining an effective amount of a low pKa acid with an amount of a water soluble salt of chlorite.
  • the overall pH for purposes of the present invention will preferably range from about 2 to about 4.5.
  • effective amount is used throughout the specification to describe a minimum amount or quantity of a component, i.e., a low pKa acid, disproportionation agent or chlorite ion included to generate an intended effect.
  • a component i.e., a low pKa acid, disproportionation agent or chlorite ion included to generate an intended effect.
  • effective amount when used to describe the low pKa acid is used to describe that amount of acid, either in dry or liq ⁇ uid form which, when combined with chlorite in solution will generate at least 1 part per million (ppm) of chlorine dioxide from chlorous acid. By definition, 1 part per million is equal to 0.0001% by weight.
  • the present invention relates to a method of producing chlorine dioxide comprising:
  • the present invention also relates to a method of producing chlorine dioxide comprising:
  • an effective amount of a salt of a chlorite preferably sodium or potassium chlorite is combined with a biologically compatible acid to produce a substantial quantity of chlorous acid.
  • a second step the chlorous acid produced is allowed to disproportionate to form chlorine dioxide.
  • preferred salts of chlorites include sodium and potas ⁇ sium chorite.
  • the biologically compatible acids according to the present invention are those acids which are generally con ⁇ sidered safe, user friendly and substantially non-toxic, for example salts of bisulfate, maleic acid and phosphoric acid, among others.
  • the concentration of chlorite salt used to generate chlorous acid in the present invention represents at least about 0.0005M and preferably ranges from about 0.002M to about 0.5M or slightly higher.
  • the amount of chlorite salt comprises at least about 0.0005M and preferably ranges from about 0.002M to about 0.2M.
  • the amount of acid, preferably biologically compatible acid, added to the chlorite salt is generally that amount effective to provide an initial pH of the reaction mixture below about 4.5, preferably lower than about 3.5 or less.
  • the low pKa acid is added in an amount which will render the initial pH in the reaction chamber, i.e., in the presence of chlorite ion, to a level below about 2.5 and most preferably to a level at or below about 2.2.
  • the initial pH generally ranges from about 3.5 to about 4.5.
  • the acid is generally provided in a concentration of about 0.00005M to upwards of about 1M, depending upon the final pH of the solution desired.
  • concentration of acid preferably ranges from about 0.01M to about 0.2 , depending upon the amount of chlorite in the composition.
  • amount of acid preferably ranges from about 0.01M to upwards of 1M or more. These concentrations will generally provide a pH of less than about 2.5 and usually less than about 2.0. Concentrations of acid producing pH , s above or below these values may also be used, depending upon the amount of chlorite to be converted to chlorine dioxide, as well as the pH desired in the reaction chamber and the ultimate con ⁇ centration of chlorine dioxide desired.
  • the chlorite salt is combined with the acid at about 15 ⁇ C to about 30 ⁇ C to produce chlorous acid. Thereafter, the chlorous acid is left to disproportionate to chlorine dioxide.
  • the disproportionation step is carried out in the same aqueous medium where the formation of chlorous acid occurs.
  • the temperature of the disproportionation step may vary, but will generally range from about 15°C to about 30°C or higher.
  • the chlorine dioxide solution may be used directly or diluted depending upon the desired use.
  • a disproportionation agent preferably in the form of an aldehyde chemical entity
  • an effective amount of an agent for disproportionating chlorous acid to chlorine dioxide is added to the solution.
  • the disproportionation agent may be added after the formation of chlorous acid, preferably the disproportionation agent is already present in the acid solu ⁇ tion when the acid solution is combined with the aqueous mix ⁇ ture of chlorite salt. In this way, as soon as chlorous acid is generated, the disproportionation reaction may be enhanced.
  • the overall result will be to shift the equilibrium toward more chlorous acid generation and consequently, more chlorine dioxide formation.
  • a disproportionation agent at least 10% and generally at least about 30-40% up to about 80% or higher of chlorite ion is converted to chlorine dioxide and chloride ion.
  • the conversion is significantly slower and is less efficient (usually sig ⁇ nificantly less than about 2% of the initial chlorite ion is converted to chlorine dioxide and/or chloride) .
  • any acid which produces an initial pH in the reaction mixture of about 4.5 or lower may be util ⁇ ized, but preferably a low pKa biologically compatible acid is used.
  • the amount of disproportionation agent used in the present invention varies depending upon the amount of chlorite ion used.
  • the amount of dis ⁇ proportionation agents used in the present invention ranges from about 10 parts per million to about 20,000 parts per mil ⁇ lion or more (about 0.001% to about 2.0% by weight).
  • the amount of disproportiona ⁇ tion agent utilized varies from about 1/10 to about 1/2 the amount of chlorite used, and preferably about 1/3 to about 1/2.
  • disproportionation agent in concentrations above and below this amount, for exam ⁇ ple, it is noted ' that at concentrations of disproportionation agent substantially below 1/10 the molar concentration of chlorite, the rate at which disproportionation of chlorous acid to chlorine dioxide occurs may be diminished. At molar concentrations of disproportionation agent significantly above about 1/2 the concentration of chlorite, residual amounts of disproportionation agent may remain in solution which could result in instability in the resulting chlorine dioxide solu ⁇ tion.
  • the amount of disproportionation agent is chosen to maximize chlorine dioxide formation and minimize the amount of residual chlorite in the chlorine dioxide mixture.
  • the apparatus as set forth in figures 1 and 2A and 2B are repre ⁇ sentative of systems that can be used to generate chlorine dioxide.
  • a chosen amount of chlorite salt is dissolved in water in vat A.
  • the chlorite salt is the sodium or potassium salt.
  • the concentra ⁇ tion of chlorite salt chosen generally ranges from about 0.001 to about 0.5 Molar (generally, for example, about 0.09g. to about 45g./liter of sodium chlorite) .
  • the chlorite salt is first added to water and dissolved.
  • the pH of the solution in Vat A may range from about 9.0 to significantly above about 10.
  • a pH above 10, for example about 10.5, is often employed.
  • a second solution, contained in Vat B, is prepared containing an effective amount of a biologically compatible acid, for example, sodium bisulfate.
  • a biologically compatible acid for example, sodium bisulfate.
  • the pH of the solution without disproportionation agent is preferably maintained below about 2.5.
  • the amount of acid chosen is that amount which is effective to produce a substan ⁇ tial quantity of chlorous acid. This amount of acid.will generally provide an initial pH of the reaction mixture in which chlorine dioxide is produced below about pH 2.5.
  • an effective amount of a disproportionation agent may be added to enhance dis ⁇ proportionation of chlorous acid to chlorine dioxide.
  • the final pH of the acid solution including disproportionation agent in this aspect of the invention is generally less than about 2.5, preferably less than about 2.0 and most preferably less than about 1.8.
  • any acid may be used including any of the aforementioned acids, among others, but preferably a low pKa biologically compatible acid is chosen.
  • Vats A and B are each stoppered so that the contents of each vat may be metered into reaction chamber C. Each or both of the Vats may be graduated.
  • the stoppering of vats A and B (valves (1) and (2)) will allow a measured or pre- easured amount of the contents of each Vat to be delivered in a controllable manner to the reaction chamber C while valve (3) is open and (4) is closed.
  • the chlorite is acidified with the low pKa biologically compatible acid to produce chlorous acid and subsequently, the generated chlorous acid is disproportionated in situ into chlorine dioxide.
  • the concentration of chlorine dioxide increases within the reaction chamber until such time as the reaction is completed.
  • the reaction(s) to produce chlorine dioxide without the aid of the disproportionation agent is slow and may require about 30 minutes or higher to be com ⁇ pleted (level off) .
  • the concentration of chlorine dioxide generated within a period of about 15 minutes ranges from about 5 ppm to upwards of 100 ppm or more.
  • the production of chlorine dioxide may be monitored photometrically at 360 nm using an extinction coef ⁇ ficient of 1250 M ⁇ 1 cm ⁇ 1 as described on pp.244-245 of "Chemistry of Chlorine Dioxide", In Progress in Inorganic Chemistry. Vol. 15, S.J. Lippard (Editor), Wiley-Interscience, New York (1972) .
  • the final concentration of chlorine dioxide in the reaction cham ⁇ ber ranges from about 80-100 parts per million (ppm) to upwards of 400 ppm.
  • reaction cham ⁇ ber C After the completion of the formation of chlorine dioxide in reaction chamber C, the contents of reaction cham ⁇ ber C are deposited into dilution tank D by opening valve 4 (valve 5 is closed) .
  • the chlorine dioxide solution from reaction chamber C is mixed with water or other aqueous solu ⁇ tion in dilution tank D (generally about a 20-40 fold dilu ⁇ tion, preferably about 30 fold) so as to create a chlorine dioxide solution with a final concentration generally ranging from slightly less than about 1 ppm to about 10 ppm, with a preferred concentration of about 1 ppm to about 5 ppm.
  • the pH of the final diluted solution of chlorine dioxide ranges from about 4.5 to about 7 with a preferred range from about 5.5 to about 6.5.
  • the chlorite part ranges from about 50 ppm to about 50,000 ppm.
  • the pH of the chlorite part may generally range from about 9.0 to about 10.8.
  • the acid part contains an effective amount of a low pKa acid, preferably non-toxic, the pH of the concentra ⁇ tion ranging from about 3.5 to about 4.5
  • an aldehyde dis ⁇ proportionation agent effective to enhance disproportionation of chlorous acid to chlorine dioxide.
  • the amount of aldehyde disproportionation agent ranges from about 20 ppm to about 40,000 ppm. .
  • any acid may be used including any of the aforementioned acids, among others, but preferably a non-toxic low pKa acid is used.
  • the final solutions of chlorine dioxide in diluted form may be used for purposes of disinfecting surfaces, espe ⁇ cially surfaces which may require reduced amounts of chlorite ion, for example, food equipment, and medical devices and den ⁇ tal equipment.
  • the solutions according to the present invention may also be used for any other known purpose especially including for drinking water.
  • the number of appli ⁇ cations of the chlorine dioxide solutions according to the present invention is believed to be larger than for solutions which are produced according to prior art methods because the solutions of the instant invention are compatible with food, medical and dental eqiupment as well as other uses known in the art.
  • Vat A See Figure 1
  • an aqueous solution containing about 0.7g./liter of pure sodium chlorite T.R.-AMC Chemicals, a Division of TR-Metro Chemicals, Inc., Ridgefield, New Jersey
  • To Vat B was added about 0.4 g./liter of potas ⁇ sium bisulfate, which produced a pH of about 1.9.
  • To this solution about 0.2g/liter of acetaldehyde was added.
  • Vat A and Vat B were emptied into the reaction chamber C by opening valves 1, 2 and 3 (valve 4 is closed) .
  • the pH of the mixture in the reaction chamber is approximately 2.2.
  • the reaction mixture was allowed to stand for a period of ten minutes after which time approximately 92% of the initial chlorite salt had been converted to chlorine dioxide (40%) and chloride ion (60%) .
  • the concentration of chlorine dioxide in the aqueous solution in the reaction cham ⁇ ber was about 110 ppm as measured spectrophotometrically at 360 nm using an extinction coefficent of 1250 M' ⁇ -cm"" 1 .
  • the concentration of chlorite ion which remains was approximately 30 ppm.
  • the concentrated chlorine dioxide solution is there ⁇ after delivered to the dilution tank D and diluted 30 fold to a final concentration of 3.5 ppm chlorine dioxide and a pH of about 6.
  • the con ⁇ centration of chlorite ion is about 1 or less ppm.
  • the rela ⁇ tively high pH of the solution is caused by the 30-fold dilu ⁇ tion, the production of water using up hydronium (H ⁇ O" 1" ) ions during the reaction and the effect of chlorine dioxide as a Lewis Acid is minimized at high dilution.
  • the fol ⁇ lowing two-part formulation when combined in about a.1:1 ratio provides a composition useful for the disinfection of hard substrates such as dental and/or medical devices.
  • the disproportionation agent in the form of an aldehyde entity namely glutaraldehyde
  • cinnamic aldehyde is used as a fragrance.
  • the resulting composition after 15 minutes has a pH of about 4.2 and produces a concentration of chlorine dioxide of about 45 ppm as measured spectrophotometrically at 360 nm (molar absorptivity of 1250 per mole/centimeter) . Within this period, about 40% of the initial chlorite is con ⁇ sumed.
  • This composition is readily applicable for disinfec ⁇ tion of hard surfaces such as dental and/or medical devices.
  • a liquid disinfectant is obtained which is useful for applications on dental and/or medical devices.
  • the disproportionation agent in the form of an aldehyde entity namely propionaldehyde
  • the resulting composition has a pH of about 3.9 and produces a concentration of chlorine dioxide of about 38 ppm as measured spectrophotometrically at 360 nm (molar absorptivity of 1250 per mole/centimeter during a period of about 10 minutes. Within this period, about 15% of the initial chlorite is consumed.
  • This composition is readily applicable for disinfection of hard surfaces such as dental and/or medical devices.
  • Example 6 In yet another embodiment related to the non-corrosive aspect according to the present invention, the following two- part formulation when combined in about a 1:1 ratio provides a composition useful for the disinfection of hard substrates such as dental and/or medical devices.
  • the pH of the composi ⁇ tion is about 4.2 and produces about 27 ppm of chlorine dioxide during an aging period of about 15 minutes.

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  • Life Sciences & Earth Sciences (AREA)
  • General Life Sciences & Earth Sciences (AREA)
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  • Inorganic Chemistry (AREA)
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Abstract

Un procédé de production permet de produire du dioxyde de chlore (C102) destiné à une solution de désinfection. Il minimise de préférence la quantité d'ions chlorate résiduels (ClO2-) ce qui permet d'utiliser cette solution de désinfection dans les industries de production et de transformation alimentaires et celles concernant l'eau potable, la production pharmaceutique ainsi que les branches médicale et dentaire apparentées. Une variante complémentaire porte sur des solutions donnant du dioxyde de chlore qui sont en pratique à l'abri de la corrosion. Dans la figure, les cuves A et B sont bouchées de manière que l'on puisse mesurer le contenu de chacune d'entre elles dans la chambre de réaction C. La cuve A contient le chlorate et la cuve B, un acide biologiquement compatible. La cuve D constitue la chambre de dilution.
EP93907256A 1992-03-04 1993-03-04 Procede pour la production du dioxyde de chlore. Withdrawn EP0629177A4 (fr)

Applications Claiming Priority (5)

Application Number Priority Date Filing Date Title
US846468 1977-10-28
US84646892A 1992-03-04 1992-03-04
US98026292A 1992-11-23 1992-11-23
US980262 1992-11-23
PCT/US1993/002015 WO1993017960A1 (fr) 1992-03-04 1993-03-04 Procede pour la production du dioxyde de chlore

Publications (2)

Publication Number Publication Date
EP0629177A1 true EP0629177A1 (fr) 1994-12-21
EP0629177A4 EP0629177A4 (fr) 1995-10-11

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EP93907256A Withdrawn EP0629177A4 (fr) 1992-03-04 1993-03-04 Procede pour la production du dioxyde de chlore.

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EP (1) EP0629177A4 (fr)
CA (1) CA2131390A1 (fr)
WO (1) WO1993017960A1 (fr)

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US6051135A (en) * 1996-02-23 2000-04-18 Water Technologies Limited Apparatus for making aqueous chlorine dioxide and apparatus for treating water with aqueous chlorine dioxide
US5855861A (en) * 1996-02-23 1999-01-05 Water Technologies Limited Method and apparatus for making aqueous chlorine dioxide
US6423675B1 (en) * 1999-11-23 2002-07-23 Diversey Lever, Inc. Cleaning-in-place composition and method for using the same
DE102012207472C5 (de) * 2012-05-04 2018-05-03 Fritz Küke Vorrichtung und Verfahren zur Herstellung wässriger Chlordioxidlösungen sowie Vorratseinheiten und Kits zur entsprechenden Verwendung
WO2021002262A1 (fr) * 2019-07-02 2021-01-07 大幸薬品株式会社 Dispositif de génération de dioxyde de chlore et procédé de génération de dioxyde de chlore

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See also references of WO9317960A1 *

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EP0629177A4 (fr) 1995-10-11
CA2131390A1 (fr) 1993-09-16
WO1993017960A1 (fr) 1993-09-16

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